1. Consider the following reaction at equilibrium: N2(g) +3H2(g)2NHs(g) AH-92 kJ
ID: 1034369 • Letter: 1
Question
1. Consider the following reaction at equilibrium: N2(g) +3H2(g)2NHs(g) AH-92 kJ The yield of ammonia can be maximized by carrying out the reaction at a) A high temperature and high pressure b) A high temperature and low pressure c) A low temperature and high pressure d) A low temperature and low pressure 2. Consider the following reaction at equilibrium N2(g) +3H2(g) 2NHs(e Increasing the pressure at a constant temperature will a) increase the yield of ammonia b) decrease the yield of ammonia c) have no effect on the yield of ammonia 3. Consider the following reaction at equilibrium: N2(g) +3H2(g) 2NH3(g) What effect will decreasing the temperature have on the system at equilibrium? a) The equilibrium constant will decrease and the reaction will proceed in the forward direction b) The equilibrium constant will decrease and the reaction will proceed in the reverse direction c) The equilibrium constant will increase and the reaction will proceed in the forward direction d) The equilibrium constant will increase and the reaction will proceed in the reverse direction e) The equilibrium constant will remain constant since it is independent of temperature, and the concentrations will not changeExplanation / Answer
1. c) low temperature and high pressure
This is because the production of ammonia is an exothermic reaction and therefore only decreasing the temperature will favour the forward reaction. Similarly, from the equation it is clear that the reaction proceeds with a decrease in the number of moles. On the reactant side there are 4 moles to 2 moles on the product side. Hence an increase in pressure will again favour the forward reaction.
2. a) increase the yield of ammonia
This is because increasing pressure favours the production of ammonia as explained above but this happens as long as the temperature is in the optimal range. When the temperature becomes very low, then the number of effective collisions become less as the molecules have lesser energy and then the yield will be small.
3. c) the equilibrium constant will increase and the reaction will proceed in the forward direction.
This is because the production of ammonia is an exothermic reaction. If the temperature is decreased the forward reaction will be favoured. Equilibrium constants are changed only by change in the temperature. Change in the concentration or the pressure does not affect the equilibrium constant.
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